Question Detail
Question
A reaction has an activation energy of 50 kJ/mol. How much faster is the reaction at 310 K compared to 300 K? (R = 8.314 J/mol·K)
Correct Answer
Option B is the correct answer.
Detailed Explanation
Using the two-point Arrhenius equation: ln(k₂/k₁) = (Ea/R)(1/T₁ - 1/T₂) = (50000/8.314)(1/300 - 1/310) = (6014)(0.0001075) = 0.647. k₂/k₁ = e⁰·⁶⁴⁷ ≈ 1.91 ≈ 1.9. Closest option is 1.8.
Hint
Convert temperatures to Kelvin and use ln(k₂/k₁) = (Ea/R)(1/T₁ - 1/T₂).